https://www.khanacademy.org/science/chemistry/oxidation-reduction/electrolytic-cell/v/introduction-to-electrolysis 2023-09-10T17:11:17.624018169Z Introduction to electrolysis Explore the world of electrochemistry with this detailed comparison of voltaic and electrolytic cells. Understand how spontaneous redox reactions in voltaic cells produce electric current, while electrolytic cells use electric current to drive non-spontaneous reactions. Learn the key differences in electrode signs and how to identify anodes and cathodes in each cell type. Jay video https://cdn.kastatic.org/googleusercontent/eEU8bcg5aEmmFPLZSFBU0grLF8hhMhMTtrzaYMHjIKmxBegLpnFtJZcqvHuWLNyUworwAT38GimVZVKN95qqx-ua Introduction to electrolysis Explore the world of electrochemistry with this detailed comparison of voltaic and electrolytic cells. Understand how spontaneous redox reactions in voltaic cells produce electric current, while electrolytic cells use electric current to drive non-spontaneous reactions. Learn the key differences in electrode signs and how to identify anodes and cathodes in each cell type. https://cdn.kastatic.org/ka-youtube-converted/1tvvSUySfls.mp4/1tvvSUySfls.mp4 415 Electrolytic cells https://www.khanacademy.org/science/ap-chemistry-beta/x2eef969c74e0d802:applications-of-thermodynamics/x2eef969c74e0d802:galvanic-voltaic-and-electrolytic-cells/v/electrolytic-cells 2022-10-05T02:43:18.611402953Z Electrolytic cells Electrolytic cells use an electric current to drive a thermodynamically unfavored redox reaction. As in galvanic cells, oxidation occurs at the anode and reduction occurs at the cathode. An application of electrolysis is the electroplating of metals, which uses an electric current to deposit a thin layer of metal onto the surface of another material. Jay video https://cdn.kastatic.org/ka_thumbnails_cache/9215a6e8-164d-494b-8e2b-878e399e344d_1280_720_base.png Electrolytic cells Electrolytic cells use an electric current to drive a thermodynamically unfavored redox reaction. As in galvanic cells, oxidation occurs at the anode and reduction occurs at the cathode. An application of electrolysis is the electroplating of metals, which uses an electric current to deposit a thin layer of metal onto the surface of another material. https://cdn.kastatic.org/ka-youtube-converted/patZ8zoemVo.mp4/patZ8zoemVo.mp4 481 Electrolytic cells https://www.khanacademy.org/science/grade-11-chemistry-snc-aligned/x203b0fc81a964b2d:electrochemistry/x203b0fc81a964b2d:electrolytic-cells/v/electrolysis-of-molten-sodium-chloride-edited 2023-09-10T17:11:17.624018169Z Electrolysis of molten sodium chloride edited Learn how electrolysis works with molten sodium chloride. See how a negative battery terminal provides electrons, causing a reduction half reaction. Understand that chloride anions oxidize to chlorine gas at the anode. Find out how to calculate the time needed to produce a certain amount of sodium using a constant current. Grasp the connection between moles of sodium and moles of electrons, and how to figure out the volume of chlorine produced. Visit us (http://www.khanacademy.org/science/healthcare-and-medicine) for health and medicine content or (http://www.khanacademy.org/test-prep/mcat) for MCAT related content. These videos do not provide medical advice and are for informational purposes only. The videos are not intended to be a substitute for professional medical advice, diagnosis or treatment. Always seek the advice of a qualified health provider with any questions you may have regarding a medical condition. Never disregard professional medical advice or delay in seeking it because of something you have read or seen in any Khan Academy video. Jay video https://cdn.kastatic.org/googleusercontent/DQNu-Wyw2Br_8NCpme5a39vjJ6NLb952LNHKSSmZ9OpHW3NM-1me8hXjONjaLJHob02gJgzx-6ycWP2B69aBbkw Electrolysis of molten sodium chloride edited Learn how electrolysis works with molten sodium chloride. See how a negative battery terminal provides electrons, causing a reduction half reaction. Understand that chloride anions oxidize to chlorine gas at the anode. Find out how to calculate the time needed to produce a certain amount of sodium using a constant current. Grasp the connection between moles of sodium and moles of electrons, and how to figure out the volume of chlorine produced. Visit us (http://www.khanacademy.org/science/healthcare-and-medicine) for health and medicine content or (http://www.khanacademy.org/test-prep/mcat) for MCAT related content. These videos do not provide medical advice and are for informational purposes only. The videos are not intended to be a substitute for professional medical advice, diagnosis or treatment. Always seek the advice of a qualified health provider with any questions you may have regarding a medical condition. Never disregard professional medical advice or delay in seeking it because of something you have read or seen in any Khan Academy video. https://cdn.kastatic.org/ka-youtube-converted/S7C-Q-RkX0I.mp4/S7C-Q-RkX0I.mp4 627 Electrolytic cells https://www.khanacademy.org/science/ap-chemistry-beta/x2eef969c74e0d802:applications-of-thermodynamics/x2eef969c74e0d802:cell-potential-and-free-energy/v/standard-cell-potential 2022-01-11T22:17:00.362877679Z Standard cell potential Standard cell potential is the potential of a cell when all reactants and products are in their standard states. The standard potential for any cell can be calculated by subtracting the standard reduction potential of the half-reaction occurring at the anode from the standard reduction potential of the half-reaction occurring at the cathode. Jay video https://cdn.kastatic.org/googleusercontent/ZCdwTudJg6e6n-P2gsaUborP4izvMsGo71pvEVlX9dNYWcLXcP7VHkWpn2grt4TUP1KoJLQP9NswyHBuBLSFTBw Standard cell potential Standard cell potential is the potential of a cell when all reactants and products are in their standard states. The standard potential for any cell can be calculated by subtracting the standard reduction potential of the half-reaction occurring at the anode from the standard reduction potential of the half-reaction occurring at the cathode. https://cdn.kastatic.org/ka-youtube-converted/nBZ4PDBhSrY.mp4/nBZ4PDBhSrY.mp4 419 Electrolytic cells